Three moles of an ideal gas are expanded isothermally and reversibly at `27^(@)C` to twice its original volume. Calculate `q, w,` and `DeltaU`.

Thermodynamics deals with energy changes of macroscopic systems. 3 moles of an ideal gas at 1.5 atm and 25^@C expands isothermally in a reversible manner to twice its original volume agaisnt an external pressure of 1 atm. Calculate the work done. [R 8.314 J//K//mol

Calculate the maximum work obtained when 0.75 mol of an ideal gas expands isothermally and reversible at 27^(@)C from 10 L to 20 L Also calculate value of q and Delta U accompanying the process.

One mole of an ideal gas is allowed to expand isothermally and reversibly at 27^@C until its volume is tripled.Find Delta S_("system") in JK^(-1)mol^(-1)

One mole of an ideal gas expands isothermally and reversibles from 5 atmospheres to 1 atmosphere at 50^(@)C . Calculate the work done.

Calculate w, q and DeltaU when 0.75 mol of anideal gas expands isothermally and revensibly at 27^(@)C from a volume of 15L to 25L

Calculate the work done when 2 moles of hydrogen expand isothermally and reversibly at 27^(@)C from 15 to 50 litres.

Three moles of an ideal gas are compressed isothermally and reversibly to a volume of 2L. The work done is 2.983 kj at 22^@C . Calculate the initial volume of the gas